Multiple Choice
According to the second law of thermodynamics, what is the natural tendency for the entropy of an isolated system to do over time?
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19. Chemical Thermodynamics
Entropy
Multiple Choice
Which of the following processes represents an increase in entropy (greater disorder) for the system?
A
Liquid water freezes to form ice at 0 °C
B
A gas is compressed to a smaller volume at constant temperature
C
Water vapor condenses to liquid water at its boiling point
D
Solid sodium chloride dissolves in water to form aqueous ions
Verified step by step guidance1
Understand the concept of entropy: Entropy is a measure of disorder or randomness in a system. Processes that increase the number of possible microstates or the freedom of movement of particles generally increase entropy.
Analyze the process 'Liquid water freezes to form ice at 0 °C': Freezing causes water molecules to become more ordered in a solid lattice, so entropy decreases.
Analyze the process 'A gas is compressed to a smaller volume at constant temperature': Compressing a gas reduces the space available for gas molecules, decreasing their randomness and thus decreasing entropy.
Analyze the process 'Water vapor condenses to liquid water at its boiling point': Condensation changes gas molecules into a more ordered liquid phase, decreasing entropy.
Analyze the process 'Solid sodium chloride dissolves in water to form aqueous ions': Dissolving a solid ionic compound into ions increases the number of particles and their freedom of movement in solution, increasing entropy.
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